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2 years ago

HHHAAAAALLLPPPP It’s due tomorrow

Chemistry

1 answer:

iris [78.8K]2 years ago

7 0

Answer:

Explanation:

Only 0.0035% of the electromagnetic spectrum is visible to the human eye

Hopefully this helped :)

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What is the volume if 1.5 mol of gas has a pressure of 700 torr at 15°C?

Tasya [4]

Answer:

V = 38.48 L

Explanation:

Given that,

No. of moles = 1.5 mol

Pressure, P = 700 torr

Temperature, T = 15°C = 288 K

We need to find the volume of the gas. The ideal gas equation is given by :

$PV=nRT\\\\V=\dfrac{nRT}{P}\\\\V=\dfrac{1.5\times 62.36\times 288}{700}\\\\V=38.48\ L$ , R = L.Torr.K⁻¹.mol⁻¹

So, the required volume is equal to 38.48 L.

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2 years ago

How many moles of Cu do you need to react with 12 moles of O2? 2Cu(s) + O2(g) 2CuO(s)

zzz [600]

Answer:

24 mol Cu

General Formulas and Concepts:

Chemistry

Stoichiometry

Explanation:

Step 1: Define

RxN: 2Cu (s) + O₂ (g) → 2CuO (s)

Given: 12 moles O₂

Step 2: Stoichiometry

$12 \ mol \ O_2(\frac{2 \ mol \ Cu}{1 \ mol \ O_2} )$ = 24 mol Cu

Step 3: Check

We are given 2 sig figs.

Our final answer is in 2 sig figs, so no need to round.

3 0

3 years ago

Use a Punnett square to predict the results of crosses

masya89 [10]

If you know the parent genotypes then you can make the Punnett square

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3 years ago

What is made out of one atom

mestny [16]

Well i know water is made out of 2 but gold is made of 1 type of atom if that helps

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3 years ago

What mass of metallic silver can form from 1.147 g of copper metal according to equation b?

Arisa [49]

Answer:

$\large\boxed{\large\boxed{3.894g}}$

Explanation:

From similar question, equation (b) is

Molecular Equation:

Cu(s) + 2AgNO₃(aq) → Cu(NO₃)₂(aq) + 2Ag(s)

Net Ionic Equation:

Cu(s) + 2Ag⁺(aq) → Cu²⁺(aq) + 2Ag(s)

1. Mole ratio:

$\dfrac{2molAg(s)}{1molCu(s)}$

2. Convert 1.147 g of Cu(s) to moles:

Atomic mass of Cu: 63.546g/mol

Number of moles = mass in grams / atomic mass

Number of moles = 1.147 g / 63.546 g/mol = 0.01805 mol Cu(s)

3. Calculate the moles of Ag(s):

$0.01805molCu(s)\times \dfrac{2molAg(s)}{1molCu(s)}=0.03610molAg(s)$

4. Convert 0.03610 mol Ag(s) to grams:

Atomic mass of Ag(s) = 107.868g/mol

Mass = 0.03610mol × 107.868g/mol = 3.894g

4 0

3 years ago