Removing the tree would decrease the water consumption but would also decrease the oxygen production.
Tropical rainforests are found in Central and South America, western and central Africa, western India, Southeast Asia, the island of New Guinea, and Australia.
Sunlight strikes the tropics almost straight on, producing intense solar energy that keeps temperatures high, between 21° and 30°C (70° and 85°F).
Deforestation has an adverse affect on air by reducing the amount of oxygen and increasing the amount of carbon dioxide as well as contributing to global warming.
Photosynthesis would produce food for the tree and as by - product, oxygen is produced.
Removing the tree would decrease the water consumption but would also decrease the oxygen production.
Learn more about tropical rainforest here:
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Answer:
Antigens are molecules capable of stimulating an immune response. Each antigen has distinct surface features, or epitopes, resulting in specific responses. Antibodies (immunoglobins) are Y-shaped proteins produced by B cells of the immune system in response to exposure to antigens.
Solution is here,
for initial case,
temperature(T1)=70°C=70+ 273=343K
vloume( V1) =45 L
for final case,
temperature( T2)=?
volume(V2)= 91.3 L
at constant pressure,
V1/V2 = T1/T2
or, 45/91.3 = 343/ T2
or, T2= (343×91.3)/45
or, T2=695.9 K = (695.9-273)°C=422.9°C
The temperature needed for a sample of gas to occupy 91.3 L, when originally it occupied 45.0 L at 70.0°C at constant pressure, is about 423.71°C.
This question pertains to the ideal gas law equation (P1V1/T1 = P2V2/T2, where P is pressure, V is volume, and T is temperature), we must first convert our temperatures to Kelvin (K) since the ideal gas law uses absolute temperature. To convert from degrees Celsius to K, add 273.15, thus 70.0°C becomes 343.15K. As the problem states pressure is constant, we can ignore that component of the equation and it simplifies to V1/T1 = V2/T2.
By rearranging the equation to solve for V2, we get V2 = V1 (T2/T1). Given the volume of the gas at the initial temperature (V1 = 45.0 L), and temperature T2 with unknown value, we rewrite the equation as T2 = (V2 * T1) / V1. Substituting the given values into the equation gives T2 = (91.3 L * 343.15K) / 45.0 L, which calculates to approximately 696.86K, converting back to Celsius gives us around 423.71°C.
So, your sample of gas would need to be heated to approximately 423.71°C in order for it to occupy a volume of 91.3 L at constant pressure.
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