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Can you give examples of carbon in our nonliving environment?

KiRa [710]

Carbon is present in many natural minerals and rocks, such as diamond, graphite, limestone. Also carbon dioxide gas, carbon monoxide gas.

3 0

3 years ago

A sample of copper absorbs 4.31E+1 kJ of heat, resulting in a temperature rise of 6.71E+1 °C. Determine the mass (in kg) of the

olga2289 [7]

Answer: 1.67 kg

Explanation:

The quantity of heat required to raise the temperature of a substance by one degree Celsius is called the specific heat capacity.

$Q=m\times c\times \Delta T$

Q = Heat absorbed= $4.31\times 10^1kJ$ = $43100J$ (1kJ=1000J)

m= mass of substance = ?

c = specific heat capacity = $0.385J/g^0C$

Change in temperature , $\Delta T=T_f-T_i=6.71\times 10^1^0C=67.1^0C$

Putting in the values, we get:

$43100J=m\times 0.385J/g^0C\times 67.1^0C$

$m=1670g=1.67kg$ (1kg=1000g)

Thus the mass (in kg) of the copper sample is 1.67

3 0

3 years ago

The following reaction shows the products when sulfuric acid and aluminum hydroxide react.

Elden [556K]

The correct answer is approximately 11.73 grams of sulfuric acid.

The theoretical yield of water from Al(OH)3 is lower than that of H₂SO₄. As a consequence, Al(OH)3 is the limiting reactant, H₂SO₄ is in excess.

The balanced equation is:

2Al(OH)₃ + 3H₂SO₄ ⇒ Al₂(SO₄)₃ + 6H₂O

Each mole of Al(OH)3 corresponds to 3/2 moles of H₂SO₄. The molecular mass of Al(OH)3 is 78.003 g/mol. There are 15/78.003 = 0.19230 moles of Al(OH)3 in the five grams of Al(OH)3 available. Al(OH)3 is in limiting, which means that all 0.19230 moles will be consumed. Accordingly, 0.19230 × 3/2 = 0.28845 moles of H₂SO₄ will be consumed.

The molar mass of H₂SO₄ is 98.706 g/mol. The mass of 0.28845 moles of H₂SO₄ is 0.28845 × 98.706 = 28.289 g

40 grams of sulfuric acid is available, out of which 28.289 grams is consumed. The remaining 40-28.289 = 11.711 g is in excess, which is closest to the first option, that is, 11.73 grams of H₂SO₄.

6 0

3 years ago

What are the hydronium and hydroxide ion concentrations in a solution whose ph is 6.52?

erica [24]

A solution with a pH of 6.52 has a hydronium ion concentration of 3.02x10-7 mol/L and a hydroxide ion concentration of 3.31x10-8 mol/L.

The hydronium ion concentration of a solution can be calculated from pH by using $10^{-pH}$ . For a pH of 6.52, hydronium ion concentration is 3.02x10-7 mol/L.

The concentration of hydroxide ions can be determined by identifying the value of pOH. The sum of pOH and pH is equal to 14, which is based on the negative logarithm of the ion-product constant of water. At a pH of 6.52, pOH is equal to 7.48.

The relationship between pOH and hydroxide ion concentration is the same as the relationship between pH and hydronium ion concentration. With this, the hydroxide ion concentration at pOH of 7.48 is $10^{-7.48}$ or 3.31x10-8 mol/L.

For more information regarding pH and pOH, please refer to the link brainly.com/question/13557815.

#SPJ4

3 0

1 year ago

Jennie decides to mix the content of her beaker with another lab group to see “the results.” Is this safe why or why not explain

Ray Of Light [21]

Answer: no

Explanation:

It could be dangerous since you don't know what substance are you adding.it may end up in an explosion

I hope this helps :)

6 0

2 years ago