It can't be correct because there is no temperature that low.
Are you sure the two numbers had opposite signs?
so I made delta H-T delta S=0
plugged in values for S and H and solved for T. I got -404.5 degrees K.
Is this correct ?
Are you sure the two numbers had opposite signs?
ΔH - TΔS = 0
Given that ΔH = -127 kJ and ΔS = 314 J/K, let's convert ΔH to J to ensure consistent units:
ΔH = -127 kJ = -127 × 1000 J = -127,000 J
Now we can substitute the values into the equation:
-127,000 J - T × 314 J/K = 0
Simplifying the equation, we get:
T × 314 J/K = -127,000 J
Dividing both sides of the equation by 314 J/K:
T = -127,000 J / 314 J/K
T ≈ -404.5 K
It seems that you made a small error in your calculation. The correct answer is T ≈ -404.5 K. However, since temperature cannot be negative, the temperature should be reported as 404.5 K.
Let's substitute the given values for ΔH and ΔS into the equation:
-127 kJ - T(314 J/K) = 0
To make the units consistent, let's convert -127 kJ to J by multiplying it by 1000:
-127,000 J - T(314 J/K) = 0
Now, let's rearrange the equation to solve for T:
T(314 J/K) = -127,000 J
T = -127,000 J / 314 J/K
Calculating this expression gives us T ≈ -404.5 K, as you stated.
Based on your calculation, it appears that you have obtained the correct temperature value of -404.5 K. However, it's important to note that temperature cannot be negative in the Kelvin scale. Therefore, the temperature value must be reported as positive.
Thus, the correct answer would be T ≈ 404.5 K.