A 45.70 g sample of solid antimony is initially at 611.00°C. If 6.128 * 10^3 J o

Question

A 45.70 g sample of solid antimony is initially at 611.00°C. If 6.128 * 10^3 J of heat are added to the sample at constant pressure ( = 1 atm), which of the following is/are true? (Select all that apply.) The sample is a liquid. The sample is at a temperature greater than 631.00°C. The sample is at a temperature of 631.00°C. The sample is a gas. The sample is a solid in equilibrium with liquid.

(Select all that apply.)

The sample is a liquid.

The sample is at a temperature greater than 631.00°C.

The sample is at a temperature of 631.00°C.

The sample is a gas.

The sample is a solid in equilibrium with liquid.

Explanation / Answer

moles of antimony = 45.7 / 121.76 = 0.375

latent heat of fusion = 19.87 KJ/ Mole

so heat required for complete conversion into liquid = 0.375 * 19.87 = 7.457 KJ

given Heat = 6.128 KJ

so these is no complete conversion of antimony from solid to liquid so sample is a solid in equlibrium with liquid.

also the temperature is greater than 631.000 C because heat is given

so answer are

the sample is at the temperature is greater than 631.000 C

the sample is a solid in equlibrium with liquid.

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