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Crazy boy [7]
3 years ago
9

Two billiard balls having masses of 0.2 kg and 0.15kg approach each other. The first ball having a velocity of 2m/s hit the seco

nd ball which is at rest. What will be the velocity of the first ball if the second ball travels at 1.5 m/s after collision?
Chemistry
1 answer:
Gekata [30.6K]3 years ago
4 0

Answer: The velocity of the first ball is 0.875 m/s if the second ball travels at 1.5 m/s after collision.

Explanation:

Given: m_{1} = 0.2 kg,      m_{2} = 0.15 kg

v_{1} = 2 m/s,    v_{2} = 0 m/s,      v'_{1} = ?,          v'_{2} = 1.5 m/s

Formula used is as follows.

m_{1}v_{1} + m_{2}v_{2} = m_{1}v'_{1} + m_{2}v'_{2}

where,

v = velocity before collision

v' = velocity after collision

Substitute the values into above formula as follows.

m_{1}v_{1} + m_{2}v_{2} = m_{1}v'_{1} + m_{2}v'_{2}\\0.2 kg \times 2 m/s + 0.15 kg \times 0 m/s = 0.2 kg \times v'_{1} + 0.15 kg \times 1.5 m/s\\0.4 kg m/s + 0 = 0.2v'_{1} + 0.225 kg m/s\\0.2v'_{1} kg = 0.175 kg m/s\\v'_{1} = \frac{0.175 kg m/s}{0.2 kg}\\= 0.875 m/s

Thus, we can conclude that the velocity of the first ball is 0.875 m/s if the second ball travels at 1.5 m/s after collision.

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Blast furnaces extra pure iron from the iron(III) oxide in iron ore in a two step sequence. In the first step, carbon and oxygen
aleksklad [387]

Answer:

The mass of O2 that will produce 10 g of Iron, Fe is 6.0 g

Note: The question is missing some details. The complete question is given below:

Blast furnaces extra pure iron from the iron (III) oxide in iron ore in a two step sequence. In the first step, carbon and oxygen react to form carbon monoxide 2C(s)+O2(e) -2CO(« In the second step, iron(III) oxide and carbon monoxide react to form iron and carbon dioxide Fe2O3(s) + 3 CO(g) → 2 Fe(s) + 3CO2(g) Suppose the yield of the first step is 90.% and the yield of the second step is 79.%. Calculate the mass of oxygen required to make 10 g of iron. Be sure your answer has a unit symbol, if needed, and is rounded to the correct number of significant digits.

Explanation:

Equation for the two reactions is given below:

Step 1: 2C(s) + O2(g) → 2CO(g)

Step 2: Fe2O3(s) + 3CO(g) → 2Fe(s) + 3CO2(g)

In the second step 3 moles of CO reacts to produce 2 moles of Fe

Molar mass of CO = 28 g/mol, molar mass of Fe = 56 g/mol

Therefore, 84 g (3 × 28) of CO will produce 112 g (2 × 56) of Fe

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However, the actual yield is 79%, therefore, 7.5 g of CO will produce 0.79 × 10 g of Fe = 7.9 g of Fe

Mass of CO that will produce an actual yield of 10 g of Fe = 7.5/7.9 × 10 = 9.50 g of CO

From the first step:

1 mole of O2 reacts to produce 2 moles of CO (molar mass of O2 = 32 g)

32 g of O2 produces 56 g (2 × 28 g) of CO

Mass of O2 that will produce 9.50 g of CO = 32/56 × 9.50 g = 5.43g

However, since the actual yield is 90%, therefore, mass of CO produced = 0.9 × 9.50 = 8.55 g of CO

Mass of O2 that will produce 9.50 g of CO = 5.43/8.55 × 9.50 g = 6.03 g

Therefore, mass of O2 that will produce 10 g of Iron, Fe is 6.0 g

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