Chapter 10, Problem 10.47PAE

The reaction ${\text{CO}}_{\text{2}}\left(\text{g}\right)+{\text{H}}_{\text{2}}\left(\text{g}\right)\to \text{CO}\left(\text{g}\right)+{\text{H}}_{\text{2}}\text{O}\left(\text{g}\right)$ is not spontaneous at room temperature but becomes spontaneous at a much higher temperature. What can you conclude from this about the signs of $\Delta \text{H}°$ and $\Delta \text{S}°$ , assuming that the enthalpy and entropy changes are not greatly affected by the temperature change? Explain your reasoning.