Using the combined gas law, the calculated volume of the gas at STP would be 0.0377 liters. If one wanted to find the volume of mole this gas at STP, then all that is required is to divide the 0.0377 liters at STP by the original number of moles of magnesium from the start of the experiment; this would yield the results at STP if one mole of magnesium was reacted, which is the same as one mole of hydrogen produced according to the chemical equation. In the end, the volume of mole of the hydrogen gas produced in this experiment would be equal to 23.6
C is plotted and fitted to a logarithmic-line to illustrate the saturation effect, shown in Figure 1. Then using equation 12.8 in the lab manual, C/Y is calculated and plotted versus C and fitted to a straight line, shown in Figure 2. From the fitted line, Ymax, which is the maximum number of moles of acetic acid that can be adsorbed on the surface of the charcoal per gram of charcoal, can be calculated from the slope. Then, using Ymax and the value of the y-intercept, K, which is the ratio between the rate constant k1 of the forward reaction (adsorption on the charcoal) and the rate constant k-1 (detachment from the charcoal), can be determined. For calculations, refer to Appendix E. Finally, multiplying Ymax by Avagadro’s number will give the number of AA molecules adsorbed on the surface of one gram of charcoal at saturation.
Explain how the molarity of the standard solution (the alkali) was calculated in the experiment (equation explained)- 0.1M of NaOH is required, this equation will be used: Concentration = moles volume This will be rearranged to find the moles needed to carry out the experiment. The concentration of the experiment using NaOH is 0.1M so we just need to rearrange the equation to find the molarity. 0.1 x 0.250 = 0.0250 moles Number of moles = mass RFM 0.0250 = mass 40 0.0250 x 40 + 1g (mass) Explain how this enabled you to accurately calculate the molarity of each acid used in the titrations (equations explained)- Molarity of the acid = molarity of the alkali x volume of the alkali volume of acid Firstly we will need to add up all of the volumes found within the titration to find an average: 13.10+13.20+13.10= 13.13 Molarity of Ethanoic acid = 0.1 x 25.00 = 0.190 mol dm-3 13.13 Molarity of Hydrochloric acid = 1.0 x 25.00 = 0.077 mol dm-3 32.53
A magnesium atom has a charge of 2+ and an oxygen atom has a charge of 2-. When the charges are balanced, the equation is MgO, one magnesium atom joined in an ionic bond with one oxygen atom. With the theoretical empirical formula found, one can now find the theoretical percent composition of MgO. The atomic molar mass of a magnesium atom is 24.31 g/mol and 16.00 g/mol for oxygen, therefore the total theoretical mass of the compound is (24.31 g/mol + 16.00 g/mol) 40.31 g/mol. The percent composition is found by dividing the element’s mass by the total mass of the
I. Title: Mass and Mole Relationships in a Chemical Reaction II. Background: Percent yield is the ratio of actual yield to theoretical yield. Amount in percent of one product formed in chemical reaction. Actual yield is the information found is experiments or is given.
Firstly, 39.15 g of water was used and molar mass of metal was determined to be 61.43 g/mol, then 50.88 g of water was used and molar mass of metal was determined to be 59.24 g/mol. If the amount of water in the calorimeter varies, and thus the heat capacity of the water would vary. Firstly, specific heat capacity of metal was determined, which depends on heat of the water mass of the water and mass of the solid, then molar mass using: MM= 25/(S.H. (J/(g℃)) ) In the Part B of the experiment q_(H_2 O) for the reaction was find to be 2279.5 joules, ∆H for the reaction = -2279.5 joules, ∆Hsolution = -455.9 joules/g. This solution reaction is exothermic; because temperature was increased meaning heat was released.
Step 1: Calculate the mean, median, and standard deviation for ounces in the bottles. Answer: Mean 14.87 Median 14.8 Standard Deveiation 0.55033 For the full calculation, refer to Appendix #1 at the end of the essay. Step 2: Create a 95% Confidence Interval for the ounces in the bottles. Answer: x ̅=14.87 ,s=0.5503 , n=30 , α=0.05 The level of confidence is at 95%. Use the following formula to determine the confidence interval: (x ̅-t_(α/2) (s/√n),x ̅+t_(α/2) (s/√n)) t_(α/2)=t_0.025=2.045 Substitute the values into the formula: (14.87-2.045(0.5503/√30),14.872.045(0.5503/√30)) = (14.665,15.075) The calculation above clearly states that the confidence interval at 95% confidence is approximately 14.665 - 15.075 ounces.
2. Explain how to determine the formula mass (mole mass) for a compound. Molar mass is the mass (in grams) of one mole of a substance. Using the atomic mass of an element and multiplying it by the conversion factor grams per mole (g/mol), you can calculate the molar mass of that element. First, find the chemical formula for the compound.
Theory The equation that was used in this experiment is % recovered = 100% X m/m0. M = mass of copper recovered and m0 = mass of original copper sample. In order to get the percent recovered, the mass must be determined. After determining the mass, you have to multiply 100% by the mass of the copper recovered divided by the mass of the original copper sample. Experiment 1.
Determination of the molar mass of a chosen compound/element Fran Jurinec 1.M Introduction Molar mass is a physical property of a chemical element or substance which shows the mass per amount of substance. My task is to determine the molar mass of a product substance from one of the following equations: a. Zn(s) + 2HCl (aq) → ZnCl2 (aq) + H2 (g) b. CaCO3 (s) + 2HCl(aq) → CaCl2 (aq) + CO2 (g) + H2O(l) c. Na2SO3 (aq) + 2 HCl (aq) → 2NaCl (aq) + S (s) + SO2 (g) For my experiment, I chose to determine the molar mass of SO2, which is a product from the 2nd equation. For this experiment I have determined the independent, dependent and controlled variables and they are: Independent variables: Volume of HCl used [ V(HCl) ] Dependent: