The reaction for the formation of ammonia is shown...

The reaction for the formation of ammonia is shown below: N2(g) + 3H2(g) ? 2 NH3(g) a) Calculate ?G° for the reaction at 500 °C using the thermodynamic values in the table below. b) At 500 °C the reaction is not spontaneous. Determine the temperature at which the reaction becomes spontaneous. Substance | ?H°f (kJ/mol) | S° (J mol?¹K?¹) N2(g) | 0 | 191.6 H2(g) | 0 | 130.7 NH3(g) | -46.1 | 192.5

Transcript

00:01 So here we need to find out about the reaction of this ammonia.

00:03 So ammonia reaction is given that is n2 plus 3h2 that gives us 2 nh3 that is ammonia.

00:11 So in this reaction what we need to find out the value of delta g we need to find out.

00:15 So for that value of delta g we very well know the formula.

00:18 The formula is delta g is equal to delta h minus t delta s.

00:23 This is our main formula.

00:25 In this formula we very well know about the delta h value so we can put the delta h values here and other than that we can put the delta temperature value.

00:35 Just we need to find the delta s value here because other values are already been provided.

00:40 So let's find the delta s value.

00:41 So delta s we will find that s of reactant minus product.

00:45 Here we can say product minus reactant.

00:48 S of product minus s of reactant.

00:52 So what is the value of product? product is nh3 so s of nh3 minus there will be the s of obviously there will be the s of value of n2 plus s of h2 that is the reactants.

01:08 So let's do here the value let's put the value.

01:11 So the s of nh3 here already been provided and that is been provided 192 .5 minus the here value of n2.

01:19 The n2 value is 191 .6 plus the h2 value is being provided 130 .7.

01:26 So let's do the calculation 192 .5 minus 322 .3.

01:32 So in the calculation we will get the value minus 129 .8...

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