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3 years ago

Which statement describes an Arrhenius acid

Chemistry

1 answer:

liq [111]3 years ago

3 0

Answer:

According to the Lewis concept, an acid is defined as a substance that accepts electron pairs and base is defined as a substance which donates electron pairs. Hence, the correct statement is arrhenius acid produces hydrogen ions in solution.

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Oxygen is a diatomic element why?

Tatiana [17]

Answer:

Oxygen exists as a diatomic molecule in nature when it is not combined with any other element. It forms O2 molecule because it is stable when it is uncombined. ... By achieving octet configuration, the diatomic elements become more stable compared to the single atom. Therefore, oxygen and hydrogen are diatomic.

Explanation:

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3 years ago

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WILL AWARD BRAINLIEST! How many moles of iron (III) oxide are produced when 0.275 moles of iron is reacted?

aev [14]

Answer:

Arrow should be yeilds, THE COEFFICIENTS are mole ratios. So every 4 moles of NH3 or ammonia produce 6 moles of H2O water

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3 years ago

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How would i calculate molecules of water produced in a reaction?

levacccp [35]

You would calculate them by dividing them and then multiplying to get the final answer

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4 years ago

Mrs. Andrews did a science demonstration with dry ice. First, she placed some dry ice inside of a balloon. Then she tied off the

RoseWind [281]

Be careful on this one! Mass is always conserved, based on the law of conservation of mass. Since their was a change in state, we went from a solid to a gas, so, the weight would be lighter, not the mass.

Same amount of mass.

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4 years ago

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What is the mass of 61.9 L of oxygen gas collected at STP?

Tcecarenko [31]

Answer:

D. 44.2 g O₂

General Formulas and Concepts:
Gas Laws

STP (Standard Conditions for Temperature and Pressure) = 22.4 L per mole at 1 atm, 273 K

Stoichiometry

Dimensional Analysis
Mole Ratio

Explanation:

Step 1: Define

Identify given.

61.9 L O₂ at STP

Step 2: Convert

We know that the oxygen gas is at STP. Therefore, we can set up and solve for how many moles of O₂ is present:

$\displaystyle 61.9 \ \text{L} \ \text{O}_2 \bigg( \frac{1 \ \text{mol} \ \text{O}_2}{22.4 \ \text{L} \ \text{O}_2} \bigg) = 2.76339 \ \text{mol} \ \text{O}_2$

Recall the Periodic Table (Refer to attachments). Oxygen's atomic mass is roughly 16.00 grams per mole (g/mol). We can use a mole ratio to convert from moles to grams:

$\displaystyle 2.76339 \ \text{mol} \ \text{O}_2 \bigg( \frac{16.00 \ \text{g} \ \text{O}_2}{1 \ \text{mol} \ \text{O}_2} \bigg) = 44.2143 \ \text{g} \ \text{O}_2$

Now we deal with sig figs. From the original problem, we are given 3 significant figures. Round your answer to the exact same number of sig figs:

$\displaystyle 44.2143 \ \text{g} \ \text{O} \approx \boxed{ 44.2 \ \text{g} \ \text{O}_2 }$

∴ our answer is letter choice D.

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Topic: AP Chemistry

Unit: Stoichiometry

6 0

2 years ago