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3 years ago

A)The lower the greenhouse gases, the higher the ocean temperature.

Chemistry

2 answers:

Lemur [1.5K]3 years ago

7 0

The lower the temperature in the beginning of the first few years.

:) Hoped this helped!!! Have a good day!!! <3

HACTEHA [7]3 years ago

6 0

The higher the greenhouse gases, the higher the ocean temperature

"The ocean absorbs most of the excess heat from greenhouse gas emissions, leading to rising ocean temperatures"

hope this helps :)

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Which is the best term to use when describing the energy of motion?

Anettt [7]

Kinetic. Transform to chemical energy in muscles

7 0

2 years ago

2 H2S(g) ⇄ 2 H2(g) + S2(g) Kc = 9.3× 10-8 at 400ºC 0.47 moles of H2S are placed in a 3.0 L container and the system is allowed t

Anon25 [30]

Answer: The concentration of hydrogen gas at equilibrium is $1.648\times 10^{-3}M$

Explanation:

We are given:

Initial moles of hydrogen sulfide gas = 0.47 moles

Volume of the container = 3.0 L

The molarity of solution is calculated by using the equation:

$\text{Molarity}=\frac{\text{Moles of solute}}{\text{Volume of the solution}}$

So, $\text{Initial molarity of hydrogen sulfide gas}=\frac{0.47}{3}=0.1567M$

The given chemical equation follows:

$2H_2S(g)\rightleftharpoons 2H_2(g)+S_2(g)$

Initial: 0.1567

At eqllm: 0.1567-2x 2x x

The expression of $K_c$ for above equation follows:

$K_c=\frac{[H_2]^2[S_2]}{[H_2S]^2}$

We are given:

$K_c=9.3\times 10^{-8}$

Putting values in above equation, we get:

$9.3\times 10^{-8}=\frac{(2x)^2\times x}{(0.1567-2x)^2}\\\\x=8.24\times 10^{-4}$

So, equilibrium concentration of hydrogen gas = $2x=(2\times 8.24\times 10^{-4})=1.648\times 10^{-3}M$

Hence, the concentration of hydrogen gas at equilibrium is $1.648\times 10^{-3}M$

7 0

3 years ago

The empirical formula for a compound is CH2. If n is a whole number, which shows a correct relationship between the molecular fo

GaryK [48]

Answer:

D)subscript of C in molecular formula = n x subscript of C in empirical formula

Explanation:

THIS IS THE COMPLETE QUESTION BELOW;

.The empirical formula for a compound is CH2. If n is a whole number, which shows a correct relationship between the molecular formula and the empirical formula? a) empirical formula mass / molecular mass = n B) molecular mass = element mass / empirical formula mass ´ 100 c) subscript of H in empirical formula = 2 subscript of H in molecular formula D) subscript of C in molecular formula = n subscript of C in empirical formula

An empirical formula can be regarded as "shorten form" of a molecular formula. Instance of this is

A compounds CH4, C2H8, C4H12... with empirical formula of CH4. In this case a constant "n" represent the difference that exist between empirical formula and molecular formula, "n" which is a whole number, molecular formula is the numerator.

Therefore, subscript of C in molecular formula = n x subscript of C in empirical formula

8 0

3 years ago

Can someone find the independent variable and the dependent variable ?

Tatiana [17]

Independent Variable here is ”Speed”, since the independent variable is defined as (what's the scientist changes or what changes on its own)... And in here, both cars were traveling at 60 mph ’at a certain point, so, one of them might speed up or stay behind/lower it's speed from the other, depending on it's driver’.

Dependent Variable here is ”Distance”, since the dependant variable is defined as (what s being studied/measured).

4 0

3 years ago

What mass of iodine would react with 48 grams of magnesium to make magnesium iodide? Mg + I2 -> MgI2

mrs_skeptik [129]

1) Chemical equation:

Mg + I2 ---> Mg I2

2) molar ratios

1 mol Mg : 1 mol I2 : 1 mol Mg I2

3) Calculate the number of moles of Mg in 48 grams

Atomic mass of Mg: 24.3 g/mol

number of moles = mass in grams / atomic mass = 48 g / 24.3 g/mol = 1.975 mol Mg

4) Use a proportion with the molar ratios

1 mol I2 / 1 mol Mg = x / 1.975 mol Mg =>

=> x = 1 mol I2 * 1.975 mol Mg / 1 mol Mg = 1.975 mol I2

5) Convert 1.975 mol I2 to grams

molar mass of I2 = 2 * 126.9 g/mol = 253.8 g/mol

mass = number of moles * molar mass = 1.975 mol * 253.8 g/mol = 501.255 g

Answer: 501 grams

6 0

3 years ago