10. What do you have to do to the coefficients of equation I below to get to equation II? i. 2 SnO2 + 4 H2 → 2 Sn + 4H2O
ii. SnO2 + 2 H2 → Sn + 2 H20

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Ответ:

beluvangel418

27.03.2020

Chemistry

480 kJ of energy is released when 3.5 mol of C_2H_4 reacts.

Explanation:

The balanced chemical reaction is:

$C_2H_4(g)+H_2(g)\rightarrow C_2H_6(g)$ $\Delta H=-137kJ$

Thus it is given that the reaction is exothermic (heat energy is released) as enthalpy change for the reaction is negative.

1 mole of C_2H_4 on reacting gives = 137 kJ of energy

Thus 3.5 moles of C_2H_4 on reacting gives = $\frac{137}{1}\times 3.5=480 kJ$ of energy

Thus 480 kJ of energy is released when 3.5 mol of C_2H_4 reacts.

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10. What do you have to do to the coefficients of equation I below to get to equation II? i. 2 SnO2 + 4 H2 → 2 Sn + 4H2O ii. SnO2 + 2 H2 → Sn + 2 H20