Question

The standard enthalpy change for the following reaction is -1.61\times 10^3 \text{ kJ} at 298 K. Si(s) + 2 F_2(g) \longrightarrow SiF_4(g) \Delta H^\circ = -1.61 \times 10^3 \text{ kJ} What is the standard enthalpy change for the reaction at 298 K? SiF_4(g) \longrightarrow Si(s) + 2 F_2(g) \text{kJ}

          The standard enthalpy change for the following reaction is -1.61\times 10^3 \text{ kJ} at 298 K.
Si(s) + 2 F_2(g) \longrightarrow SiF_4(g)
\Delta H^\circ = -1.61 \times 10^3 \text{ kJ}
What is the standard enthalpy change for the reaction at 298 K?
SiF_4(g) \longrightarrow Si(s) + 2 F_2(g)
\text{kJ}

The standard enthalpy change for the following reaction is -1.61×10^3 kJ at 298 K.
Si(s) + 2 F2(g) ⟶SiF4(g)
ΔH^∘= -1.61 ×10^3 kJ
What is the standard enthalpy change for the reaction at 298 K?
SiF4(g) ⟶Si(s) + 2 F2(g)
kJ

Added by Julie W.

Chemistry: Structure and Properties

Nivaldo Tro 2nd Edition

Instant Answer

Solved by Expert David Collins

03/20/2023

Step 1

Step 1: The second reaction is the reverse of the first reaction. Show more…

Show all steps

Thanks for your feedback!

The standard enthalpy change for the following reaction is -1.61×10^3 kJ at 298 K. Si(s) + 2 F2(g) → SiF4(g) ΔΗ° = -1.61×10^3 kJ What is the standard enthalpy change for the reaction at 298 K? SiF4(g) → Si(s) + 2 F2(g) KJ