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dalvyx [7]
3 years ago
11

Given that a 3cm lenght of magnesium weights approximately 0.04g, calculate the number of moles of acid that reacted with the 9c

m piece of magnesium ribbon.​
Chemistry
1 answer:
pychu [463]3 years ago
7 0
Iiiiiiiiiiiiooooooopp.
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Please do this please please it depends on my grades
solong [7]

Answer:

I think it's

Explanation:

It's A and C

I guess...

Sry if I'm wrong

4 0
2 years ago
Read 2 more answers
Based on the activity series, which one of the reactions below will occur (Spontaneous)? A. Mn (s) + NiCl2 (aq) → MnCl2 (aq) + N
kap26 [50]

Answer:

Mn (s) + NiCl2 (aq) → MnCl2 (aq) + Ni

Explanation:

The order of displacement of metals from aqueous solution by another metal is defined by the activity series of metals.

The activity series arranges metals in order of reactivity and increasing electrode potentials. The less negative the electrode potential of a metal is, the less reactive it is and the lower it is found in the activity series.

Nickel has a less negative electrode potential than manganese hence it is displaced from an aqueous solution of its salt by manganese spontaneously.

8 0
3 years ago
Acids react with
Verdich [7]
Water is produce bases and says
6 0
3 years ago
Calculate the mass of butane needed to produce 97.4 g of carbon dioxide. Express your answer to three significant figures and in
Vsevolod [243]

Answer:

32.1 g

Explanation:

Step 1: Write the balanced combustion reaction

C₄H₁₀ + 6.5 O₂ ⇒ 4 CO₂ + 5 H₂O

Step 2: Calculate the moles corresponding to 97.4 g of CO₂

The molar mass of CO₂ is 44.01 g/mol.

97.4 g × 1 mol/44.01 g = 2.21 mol

Step 3: Calculate the moles of butane that produced 2.21 moles of carbon dioxide

The molar ratio of C₄H₁₀ to CO₂ is 1:4. The moles of C₄H₁₀ required are 1/4 × 2.21 mol = 0.553 mol

Step 4: Calculate the mass corresponding to 0.553 moles of C₄H₁₀

The molar mass of C₄H₁₀ is 58.12 g/mol.

0.553 mol × 58.12 g/mol = 32.1 g

4 0
3 years ago
What is the mass of 1.84 mol NaCl? Give your
Sphinxa [80]

Answer:

108 g

Explanation:

3 0
3 years ago
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