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3 years ago

Can someone help me match them

Chemistry

1 answer:

ozzi3 years ago

6 0

1: shield volcano: 2

2: cinder cone volcano :3

3 : composite volcano : 1

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(will give brainliest) show your work. How many grams of Copper(I) nitrate, CuNO3 are required to produce 88.0 grams of aluminum

ValentinkaMS [17]

Based on the stoichiometry of the reaction, 156.114 g of CuNO3 are required to produce 88.0 grams of aluminum nitrate, Al(NO3)3.

<h3>What is stoichiometry of a reaction?</h3>

The stoichiometry of a reaction is the molar ratio in which reactants combine to form products.

The stoichiometry of the reaction shows that 6 moles of copper (i) nitrate produces 2 moles of aluminium nitrate.

molar mass of Copper(I) nitrate, CuNO3 = 126 g

molar mass of aluminum nitrate, Al(NO3)3 = 213 g

88.0 g of aluminum nitrate, Al(NO3)3 = 88.0/213 moles = 0.413 moles

0.413 moles of Al(NO3)3 will be produced by 0.413 ×6/3 = 1.239 moles of CuNO3

Mass of 1.239 moles of CuNO3 = 1.239 × 126 = 156.114 g of CuNO3

Therefore, 156.114 g of CuNO3 are required to produce 88.0 grams of aluminum nitrate, Al(NO3)3.

Learn more about stoichiometry at: brainly.com/question/16060223

Therefore, 156.114 g of CuNO3

4 0

2 years ago

How do molecular bonds form?

vaieri [72.5K]

Answer:

"A molecular, or covalent bond, is formed when atoms bond by sharing pairs of electrons. This sharing can occur from atom to atom, or from an atom to another molecular bond."

Explanation:

Google

8 0

3 years ago

Read 2 more answers

name the following chemical compound. p2o5 a. diphosphorus pentoxide b. diphosphorous tetraoxide c. phosphorous(ii) tetraoxide d

RUDIKE [14]

Diphosphorus pentoxide

5 0

3 years ago

Help I need to show work!

lubasha [3.4K]

Answer:

a. Combustion.

b. $m_C=3.057gC$

c. $m_H=3.67gH$

Explanation:

Hello.

a. In this case, given the reaction by which propane is converted into carbon dioxide and water:

$C_3H_8+5O_2 \rightarrow 3CO_2+4H_2O$

It is known as a combustion reaction since it is about a fuel (here propane) which is burnt by the oxygen contained in the air (21%).

b. Since the carbon dioxide contains all the carbon in the products based on the law of conservation of mass, the yielded grams are computed via a mole mass relationship:

$m_C=11.21gCO_2*\frac{12gC}{44gCO_2}=3.057gC$