Help asap i have to get a good grade on this

**PLATO QUESTION, PLEASE ANSWER CORRECTLY, THANK YOU**

marta [7]

PLATO ANSWERS:

A. Which source of electricity generation caused the most emissions?

B. What types of industries are responsible for greenhouse gas emissions?

C. What caused the dip in greenhouse gas emissions in transportation after 2007?

Hope I helped some, Have a great day!

7 0

2 years ago

Read 2 more answers

How many moles of hydrogen molecules (h2) would be required to produce two moles of hydrogen peroxide (h2o2)?

SashulF [63]

Their should be two molecules of hydrogen (h2) to produce 2 moles of h2O2

3 0

3 years ago

I WILL GIVE 50 POINTS AND BRAINLIEST What is the volume of 41.2g argon at stp???

iragen [17]

Answer:

1645.86

Explanation:

4 0

2 years ago

An atom of boron has an atomic number of 5 and an atomic mass of 11. The atom contains:. . A. 5 protons, 6 electrons, and 5 neut

Mars2501 [29]

C. 5 protons, 5 electrons, and 6 neutrons

8 0

3 years ago

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Hydrogen peroxide decomposes to water and oxygen at constant pressure by the following reaction: 2H2O2(l) → 2H2O(l) + O2(g) ΔH =

Mashcka [7]

Answer: The amount of heat released is -7.203 kJ

Explanation:

The given chemical equation follows:

$2H_2O_2(l)\rightarrow 2H_2O(l )+O_2(g);\Delta H=-196kJ$

To calculate the enthalpy change for 1 mole of the hydrogen peroxide, we use unitary method:

When 2 moles of hydrogen peroxide is reacted, the enthalpy of the reaction is -196 kJ

So, when 1 mole of hydrogen peroxide will react, the enthalpy of the reaction will be $\frac{-196}{2}\times 1=-98kJ$

To calculate the number of moles, we use the equation:

$\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}$

Given mass of hydrogen peroxide = 2.50 g

Molar mass of hydrogen peroxide = 34 g/mol

Putting values in above equation, we get:

$\text{Moles of hydrogen peroxide}=\frac{2.50g}{34g/mol}=0.0735mol$

To calculate the heat of the reaction, we use the equation:

$\Delta H_{rxn}=\frac{q}{n}$

where,

$q$ = amount of heat released

n = number of moles = 0.0735 moles

$\Delta H_{rxn}$ = enthalpy change of the reaction = -98 kJ/mol

Putting values in above equation, we get:

$-98kJ/mol=\frac{q}{0.0735mol}\\\\q=(-98kJ/mol\times 0.0735mol)=-7.203kJ$

Hence, the amount of heat released is -7.203 kJ

8 0

3 years ago