A 1.43 g sample of a mixture of magnesium carbonate and magnesium hydroxide is treated with nitric acid. The reaction produces 0.236 L of gas at 28.3°C and 743 torr.
(a) Write a balanced chemical equation for the reaction, assuming there are equal moles of each component. Hint: Write each reaction separately; then, combine them.
(b) Write the net ionic reaction for the neutralization.
(c) In reality, there are not equal moles of each substance. Assuming that the reaction completed, calculate the percentage by mass of magnesium carbonate in the sample.
(d) If the sample was treated with 30.45 mL of acid, what is its concentration?
(e) If the heat of reaction is Hrxn = -75 kJ/mol acid, how much heat must be added or removed by the surroundings to maintain a constant temperature of 28.3 °C?