Chapter 5 - Chapter 5 1. It is found that 6.00 g of...

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Chapter 5 1. It is found that 6.00 g of potassium metal reacts with excess water to release 29.8 kJ of heat. This means that, for the reaction 2 K(s) + 2 H 2 O( l ) KOH(aq) + H 2 (g) the enthalpy of reaction (per mole of H 2 produced) is A. Δ H = +189 kJ B. Δ H = 4.97 kJ C. Δ H = +388 kJ D. Δ H = 194 kJ E. None of the above is within 1% of the correct answer 2. Given the following reactions and their enthalpy changes 2 C 2 H 2 (g) + 5 O 2 (g) 4 CO 2 (g) + 2 H 2 O(l) Δ H RXN = –2599.2 kJ C(s) + O 2 (g) CO 2 (g) Δ H RXN = –393.5 kJ 2 H 2 (g) + O 2 (g) 2 H 2 O(l) Δ H RXN = –571.8 kJ Calculate Δ H ° f for acetylene, C 2 H 2 (g). A. 620.2 kJ B. 620.2 kJ C. 453.4 kJ D. 226.7 kJ E. None of the above is within 10% of the correct answer 3. The value of Δ H ° for the following reaction is –62.1 kJ. What is the value of Δ H ° f (in kJ/mol) for HCl(g)? SO
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Chapter 5 - Chapter 5 1. It is found that 6.00 g of...

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