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Brilliant_brown [7]
4 years ago
8

We could avoid a large increase in temperature if greenhouse emissions peaked by the year _____.

Chemistry
1 answer:
Naya [18.7K]4 years ago
4 0

Answer:

2036

Explanation:

  • Greenhouse gases also called GHGs are those gases found on the earth that is a product of the earth absorption and radiation of heat energy from the sun that creates a heating effect some of them are methane, carbon water vapor, ozone and nitrogen oxides.
  • The atmosphere of other planets also consists of greenhouse gases, but the impact of humans on the earth has created these gases to a certain extent that global temperatures are raised to dangerous levels.  
  • Thought the peak greenhouse gas effects and global warming process have already started in 2010, the impact of the industrial revolution has increased the atmospheric carbon content to about 50 % since the ancient times from 280 to 415 ppm in 2019.
  • At present the temperature has increased to 3 degrees from earlier times, the <u>United Nations IPCC claims that the upper limit which is to be avoided at all costs is until the year 2036</u>. Which is marked as a significant year for the upper atmospheric changes
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Calculate the amount of heat needed to boil 120.g of acetic acid (HCH3CO2), beginning from a temperature of 16.7°C.
evablogger [386]

Answer:

The total amount of heat needed = 72.2116  kJ

Explanation:

Given that ;

the mass of acetic acid = 120.0 g

The initial temperature T_1 = 16.7 °C  = (16.7 + 273.15 ) K = 298.85 K

The standard molar mass of acetic acid = 60.052  g/mol

Thus ; we can determine the number of moles of acetic acid;

number of moles of acetic acid = mass of acetic acid/ molar mass of acetic acid

number of moles of acetic acid = 120.0 g/ 60.052 g/mol

number of moles of acetic acid =  1.998 moles

For acetic acid:

The standard boiling point  T_2 = 118.1 °C = ( 118.1 + 273.15 ) K = 391.25 K

The enthalpy of vaporization of acetic acid \Delta H_{vap} = 23.7 kJ/mol

The heat capacity of acetic acid   c = 2.043  J/g.K

The change in temperature Δ T = T_2 - T_1

Δ T = (391.25 - 289.85)K

Δ T = 101.4 K

The amount of heat needed to bring the liquid acetic acid at 16.7°C to its boiling point is ;

q = mcΔT

From our values above;

q = 120 g ×  2.043  J/g.K × 101.4 K

q = 24859.2  J

q = 24859 /1000 kJ

q = 24.859 kJ

we have earlier calculated our number of moles o f acetic acid to be 1.998 moles;

Thus;

The needed amount of heat = \Delta_{vap} *numbers \ of  \ moles

The needed amount of heat = 23.7 \ kJ/mol * 1.998 \ moles

The needed amount of heat = 47.3526 kJ

Hence;

The total amount of heat needed = 24.859 kJ + 47.3526 kJ

The total amount of heat needed = 72.2116  kJ

4 0
3 years ago
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