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katrin2010 [14]
3 years ago
7

Find the volume of a sample of aluminum if its density is 2.699 g/cm3 and its mass is 26.0g?

Chemistry
1 answer:
dmitriy555 [2]3 years ago
7 0
I got 9.63 as the answer.

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Subject is mental flexiblity
lubasha [3.4K]

Answer:

A pineapples bananas

because you have to peel them

5 0
2 years ago
How many moles of water are required to produce 2.15 mol oxygen gas in this reaction
Gwar [14]
How am I supposed to know >:(
8 0
3 years ago
An ice cube of mass 8.5g is added to a cup of coffee, whose temperature is 95 degrees Celcius and which contains 120 g of liquid
Ne4ueva [31]

Answer:

\text { The temperature of the coffee after the ice melts is } 83.4^{\circ} \mathrm{C}

Explanation:

Firstly determine heat absorbed by the ice-cube while it is melting:

\mathrm{q}_{\mathrm{ice}}=\frac{8.5 \mathrm{gm} \text { ice } \times 1 \mathrm{mol} \text { ice } \times 6 \mathrm{kJ}}{18.0152 \mathrm{gm} \text { ice } \times 1 \mathrm{mol} \text { ice }}

\mathrm{q}_{\mathrm{ice}}=\frac{51}{18.0152}

\mathbf{q}_{\text {ice }}=2.83 \mathrm{kJ}

\text { Now heat emitted by the coffee while ice is melting: } q_{\varepsilon}=-q_{\mathrm{ice}}=-2.83 \mathrm{kJ}

Now the temperature of the coffee when the ice has melted:

\mathrm{q}_{\mathrm{c}}=\mathrm{m}(\Delta \mathrm{T})(\mathrm{C})

\Delta \mathrm{T}=\frac{q_{c}}{m c}

\mathrm{T}_{\mathrm{f}}-\mathrm{T}_{\mathrm{i}}=\frac{q_{c}}{m c}

\mathrm{T}_{\mathrm{f}}=\left(\frac{q_{\mathrm{c}}}{m c}\right)+\mathrm{T}_{\mathrm{i}}

\mathrm{T}_{\mathrm{f}}=\frac{-2.83 \times 10^{3} \mathrm{J}}{120 \mathrm{gm}\left(4.18 \mathrm{J} / \mathrm{gm} .^{\circ} \mathrm{C}\right)}+95^{\circ} \mathrm{C}

T_{f}=\frac{-2.83 \times 10^{3}}{501.6}+95

\mathrm{T}_{\mathrm{f}}=-5.64+95

\mathrm{T}_{\mathrm{f}}=89.37^{\circ} \mathrm{C}

Since both the substances eventually reach thermal equilibrium then they both must have the same final temperature.

\text { As } \mathrm{q}_{\mathrm{w}}=-\mathrm{q}_{\mathrm{c}}

By solving this, equation achieved is:

\mathrm{T}_{\mathrm{f}}=\frac{\mathrm{m}_{\mathrm{w}} \mathrm{T}_{\mathrm{iv}} \mathrm{C}_{\mathrm{w}}+\mathrm{m}_{\mathrm{c}} \mathrm{T}_{\mathrm{ic}} \mathrm{C}_{\mathrm{c}}}{\mathrm{m}_{\mathrm{w}} \mathrm{C}_{\mathrm{W}}+\mathrm{m}_{\mathrm{c}} \mathrm{C}_{\mathrm{c}}}

\mathrm{T}_{\mathrm{f}}=\frac{(8.5 \mathrm{gm})\left(0.0^{\circ} \mathrm{C}\right)\left(4.18 \mathrm{J} / \mathrm{gm} .^{\circ} \mathrm{C}\right)+(120 \mathrm{gm})\left(89.37^{\circ} \mathrm{C}\right)\left(4.18 \mathrm{J} / \mathrm{gm} .^{\circ} \mathrm{C}\right)}{(8.5 \mathrm{gm})\left(4.18 \mathrm{J} / \mathrm{gm} .^{\circ} \mathrm{C}\right)+(120 \mathrm{gm})\left(4.18 \mathrm{J} / \mathrm{gm} .^{\circ} \mathrm{C}\right)}

\mathrm{T}_{\mathrm{f}}=\frac{0+44827.992}{35.53+501.6}

\mathrm{T}_{\mathrm{f}}=\frac{44827.992}{537.13}

\mathrm{T}_{\mathrm{f}}=83.4^{\circ} \mathrm{C}

7 0
3 years ago
Calculate δg o for the reaction between al(s) and cd2+(aq). enter your answer in scientific notation.
Sauron [17]
The reaction between Al(s) and Cd²⁺(aq) is:
Al(s) + Cd²⁺(aq) → Al³⁺(aq) + Cd(s)

The half reactions are:
Al³⁺(aq) + 3 e⁻ → Al(s)           E⁰ = -1.66 V
Cd²⁺(aq) + 2 e⁻ → Cd(s)        E⁰ = -0.40 V

Reverse the first equation and add to the second one
2 Al(s) + 3 Cd²⁺(aq) → 2 Al³⁺(aq) + 3 Cd(s)

So, the overall cell potential is:
E⁰cell = 1.66 - 0.40 = 1.26 V

Free energy of the reaction is:
ΔG⁰ = -n F E⁰cell
        = - 6 mol e⁻ * (96485 C / mol e⁻) * (1.26 V)
        = - 7.29 x 10⁵ J

5 0
3 years ago
Methane (ch4) is a greenhouse gas. how many hydrogen atoms are in 1.4 moles of methane?
kherson [118]

The answer is:

There are 3.6 X 10^24 hydrogen atoms.

The explanation:

1.4 moles of methane will contain 1.4*Avogadro's number

                                       = 1.4*(6.02 X 10^23) =  8.4 X 10^23 methane molecules. But, since the formula for methane is CH4, there are 4 hydrogen atoms for each methane molecule. Thus, 1.4 moles of methane contain

4*(8.4 X 10^23) = 3.6 X 10^24 hydrogen atoms.

8 0
3 years ago
Read 2 more answers
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