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Using the following thermochemical equation, calculate how much heat is associated with the decomposition of 4.00 moles of NH4Cl. NH3(g) + HCl(g) è NH4Cl(s) ΔH = -176 kJ A) 5000 B) 740 C) 407 D) 704
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Using the following thermochemical equation, calculate how much heat is associated with the decomposition of 4.00 moles of NH4Cl.

NH3(g) + HCl(g) è NH4Cl(s) ΔH = -176 kJ

A) 5000
B) 740
C) 407
D) 704

User Sarbjit
by
5.7k points

2 Answers

2 votes

Answer:

D - 704

Step-by-step explanation:

The balanced thermochemical equation relates the energy change to moles, not grams, so we first convert the amount of NH4Ck to moles and then use the thermochemical equation to determine the energy change:

4.00 mole NH4Cl x (-176 ÷ 1 mole NH4Cl)

= -704

User Crlsrns
by
5.4k points
2 votes

Answer:

D

Step-by-step explanation:


4 * - 176 = - 704

User IRoygbiv
by
5.2k points
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