The initial temperature of three moles of oxygen gas is 30.0C, and its pressure is 7.40...

 

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The initial temperature of three moles of oxygen gas is 30.0°C, and its pressure is 7.40 atm. (a) What will its final temperature be when heated at constant volume so the pressure is two times its initial value? 333 °C (b) Now the volume of the gas is also allowed to change. Determine the final temperature if the gas is heated until the pressure and the volume are tripled. Apply the ideal gas law to the initial and final situations. Check temperature unit for consistency.°C 9. [0.97/2 Points] DETAILS PREVIOUS ANSWERS MY NOTES ASK YOUR Burns produced by steam at 100°C are much more severe than those produced by the same mass of 100°C water. To verify this, do the following. (a) Calculate the heat (in kcal) that must be removed from 4.00 g of 100°C water to lower its temperature to 52.0°C. 0.19 kcal (b) Calculate the heat (in kcal) that must be removed from 4.00 g of 100°C steam to condense it and lower its temperature to 52.0°C. 2.35 kcal (c) Calculate (in kg) the mass of human flesh that the heat produced in each case can raise from the normal 37.0°C to 52.0°C. (Flesh is badly damaged at 50.0°C.) steam X kg water kg Additional Materials Activate Windows O Reading Go to Settings to activat The initial temperature of three moles of oxygen gas is 30.0°C, and its pressure is 7.40 atm. (a) What will its final temperature be when heated at constant volume so the pressure is two times its initial value? 333 °C (b) Now the volume of the gas is also allowed to change. Determine the final temperature if the gas is heated until the pressure and the volume are tripled. Apply the ideal gas law to the initial and final situations. Check temperature unit for consistency.°C 9. [0.97/2 Points] DETAILS PREVIOUS ANSWERS MY NOTES ASK YOUR Burns produced by steam at 100°C are much more severe than those produced by the same mass of 100°C water. To verify this, do the following. (a) Calculate the heat (in kcal) that must be removed from 4.00 g of 100°C water to lower its temperature to 52.0°C. 0.19 kcal (b) Calculate the heat (in kcal) that must be removed from 4.00 g of 100°C steam to condense it and lower its temperature to 52.0°C. 2.35 kcal (c) Calculate (in kg) the mass of human flesh that the heat produced in each case can raise from the normal 37.0°C to 52.0°C. (Flesh is badly damaged at 50.0°C.) steam X kg water kg Additional Materials Activate Windows O Reading Go to Settings to activat