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:CO2(g) will be formed at a faster rate in experiment 2 because more H+ particles can react per unit time
Explanation:
Answer:
Explanation:
Given that
Mass ,m= 8.8 x 10¹³
Speed ,v= 33 km/s
We know that 1 km= 1000 m
v= 33 x 10³ m/s
As we know that kinetic energy given as
Now by putting the values in the above equation
Therefore we can say that the kinetic energy will be
Biosphere. it is a place where plant's and animals live together and they r interconnected to eachother
