General Chemistry Answers

empty beakers mass: 137.70g

beaker with hydrated copper (ii) sulfate: 140.70g

hydrated copper (ii) sulfate: 3.0g

beaker with anhydrous copper (ii) sulfate: 139.64g

a) Determine the amount (in mol) of water of hydration in your sample.

b) Determine the amount (in mol) of anhydrous copper (ii) sulfate in your sample.

Should your calculated value for the percentage of water be similar or different to those determined by other groups? Explain? (this is a question for a hydrate lab)

determine the mass of water and mass of anhydrous copper (ii) sulphate produced.

Chemistry Student Ana had a chance to look over the results for her entire class

The first question) Calculate the percentage atom economy of using copper oxide and sulfuric acid to make copper sulfate:

CuO(s) + H₂SO₄(aq) --> CuSO₄(aq) + H₂O(l)

Give your answer to 3 significant figures

second question) Calculate the atom economy to make copper nitrate:

CuCO₃(s) + 2HNO₃(aq) --> Cu(NO₃)₂(aq) + CO₂(g) + H₂O(l)

Give your answer to 3 significant figures

The rate constants of some reactions double with every 10-degree rise in temperature. Assume that a reaction takes place at 295 K and 305 K. What must the activation energy be for the rate constant to double as described?

Given the same reactant concentrations, the reaction

at 250°C is times as fast as the same reaction at 150°C. Calculate the activation energy for this reaction. Assume that the frequency factor is constant.

The rate constant for the second-order reaction

is at 10°C. (a) Starting with a concentration of 0.086 M, calculate the concentration of NOBr after 22 s. (b) Calculate the half-lives when and .

1. Consider the reaction

The rate of the reaction is when the concentration of A is 0.35 M. Calculate the rate constant if the reaction is (a) first order in A and (b) second order in A.