The 7160 cal energy is required to melt 10. 0 g of ice at 0. 0°C, warm it to 100. 0°C and completely vaporize the sample.
Calculation,
Given data,
Mass of the ice = 10 g
Temperature of ice = 0. 0°C
- The ice at 0. 0°C is to be converted into water at 0. 0°C
Heat required at this stage = mas of the ice ×latent heat of fusion of ice
Heat required at this stage = 10 g×80 = 800 cal
- The temperature of the water is to be increased from 0. 0°C to 100. 0°C
Heat required for this = mass of the ice×rise in temperature×specific heat of water
Heat required for this = 10 g×100× 1 = 1000 cal
- This water at 100. 0°C is to be converted into vapor.
Heat required for this = Mass of water× latent heat
Heat required for this = 10g ×536 =5360 cal
Total energy or heat required = sum of all heat = 800 +1000+ 5360 = 7160 cal
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Answer:
B
Explanation:
B is the best showing of a chemical reaction out of the choices
Density = mass/volume
D = 500 g /200 cm^3
D = 2.5 g/cm^3
hope this helps!
Answer:
No, the only way they can be separated is through chemical methods. ... A compound is made up of two or more elements that are chemically combined and elements are combined to form a compound.
Explanation:
Explanation:
1 sulfur dioxide 2 monosulfur dinitride 10 nitrogen dioxide
