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2 years ago

How does more greenhouse gases in the Earth's atmosphere affect earth's temperature?

Chemistry

2 answers:

Mumz [18]2 years ago

5 0

Explanation:

Greenhouse gasses in Earth's atmosphere affect Earth's temperature by making it hotter. Greenhouse gasses make the Earth warmer by trapping heat. You can think of greenhouse gasses as Earth's blanket.

vitfil [10]2 years ago

4 0

Answer:

It effects the earth when we have more greenhouse gasses in the earth's atmosphere because it makes the earth more warmer which will cause more sunlight to hit earth because there is more heat near the earth's surface, and this will cause the temperatures to rise really high because of the heat.

Hope this helps!

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Which step of the scientific method involves identifying variables

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Testing a typothesiss

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3 years ago

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How many grams of KCl 03 are needed to produce 6.75 Liters of O2 gas measured at 1.3 atm pressure and 298 K?

Nina [5.8K]

11.48-gram of $KCl0_3$ are needed to produce 6.75 Liters of $O_2$ gas measured at 1.3 atm pressure and 298 K

<h3>What is an ideal gas equation?</h3>

The ideal gas law (PV = nRT) relates the macroscopic properties of ideal gases. An ideal gas is a gas in which the particles (a) do not attract or repel one another and (b) take up no space (have no volume).

First, calculate the moles of the gas using the gas law,

PV=nRT, where n is the moles and R is the gas constant. Then divide the given mass by the number of moles to get molar mass.

Given data:

P= 1.3 atm

V= 6.75 Liters

n=?

R= $0.082057338 \;L \;atm \;K^{-1}mol^{-1}$

T=298 K

Putting value in the given equation:

$\frac{PV}{RT}=n$

$n= \frac{1.3 \;atm\; X \;6.75 \;L}{0.082057338 \;L \;atm \;K^{-1}mol^{-1} X 298}$

Moles = 0.3588 moles

Now,

$Moles = \frac{mass}{molar \;mass}$

$0.3588 moles = \frac{mass}{32}$

Mass= 11.48 gram

Hence, 11.48-gram of $KCl0_3$ are needed to produce 6.75 Liters of $O_2$ gas measured at 1.3 atm pressure and 298 K

Learn more about the ideal gas here:

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1 year ago

At 100°C, Kp = 60.6 for the reaction2NOBr(g) ⇄ 2NO(g) + Br₂(g) In a given experiment, 0.10 atm of each component is placed in a

Mariana [72]

The system is not at equilibrium.

The reaction will proceed to the right to attain the equilibrium.

Let's consider the following reaction.

2 NOBr(g) ⇌ 2 NO(g) + Br₂(g)

The pressure equilibrium constant (Kp) is 60.6. To determine if the system is at equilibrium when the pressure of each component is 1.75 atm, we have to calculate the reaction quotient (Q) and compare it with Kp.

Q = [NO]².[Br₂] / [NOBr]²

Q = (1.75)².(1.75) / (1.75)²

Q = 1.75

Since Q ≠ Kp, the system is not at equilibrium.

Since Q < Kp, the reaction will proceed to the right to attain the equilibrium.

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7 months ago

Please answer the questions in the pic! 15 points!

lesya [120]