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3 years ago

For the reaction 2 H2(g) + O2(g) → 2 H2O(g), how many liters of water can be made from 5.0 L of

Chemistry

1 answer:

Lana71 [14]3 years ago

6 0

Answer: 5L O2 x 1 mol O2/ 22.4L O2 x 2 mol H20/ 1 mol O2 x 22.4L H20/ 1 mol H20 = 10 L H2O

Explanation:

For future reference though, since its at STP that means that the coefficient are in proportion. Since oxygen has a coefficient of 1 and water has a coefficient of 2 for every 1 liter of oxygen there is 2 liters of water. Hence you started with 5 liters and ended with 10

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Did you write these compounds? KBr 2 NH₂OH 2HNO3

Orlov [11]

The missing components of the neutralisation reaction include the following:

KBr
KBr 2NH4OH
KBr 2NH4OH2HNO2

<h3>What is neutralisation reaction?</h3>

Neutralisation reaction is defined as the type of reaction that leads to the formation of salt and water when an acid and a base reacts.

From the reactions given the missing components are replaced as follows:

HBr + KOH --> KBr + H2O

H2SO4 + 2NH4OH --> (NH4)2SO4 + 2H2O

2HNO3 + Mg(OH)2 --> Mg(NO3)2 + 2H2O

Learn more about acids here:

brainly.com/question/26353151

#SPJ1

7 0

2 years ago

One of the intermediates in the synthesis of glycine from ammonia, carbon dioxide, and methane is aminoacetonitrile, C2H4N2.

mart [117]

Answer:

You could expect 3.48 grams of C₂H₄N₂

Explanation:

You must start by stating the chemical equation for the reaction of ammonia, carbon dioxide, and methane to produce aminoaceto nitrile.

1. Word equation:

Ammonia + Carbon dioxide + Methane → Aminoacetonitrile + Water

2. Balanced chemical equation:

$8NH_3+5CO_2+3CH_4\rightarrow 4C_2H_4N_2 +10H_2O$

3. Convert the mass of each reactant into number of moles:

Formula:

Number of moles = mass in grams/molar mass

2.11g NH₃

Number of moles = 2.11g / 17.03g/mol = 0.124 mol NH₃

14.9g CO₂

Number of moles = 14.9g/44.01g/mol = 0.339 mol CO₂

1.75g CH₄

Number of moles = 1.75g/16.04g/mol = 0.109 mol CH₄

4. Theoretical mol ratio

From the balanced chemical equation, using the coefficientes:

$8molNH_3:5molCO_2:3molCH_4:4molC_2H_4N_2:10molH_2O$

5. Limiting reagent

The available amounts of the reactants are:

0.124 mol NH₃

0.339 mol CO₂

0.109 mol CH₄

Fom the theoretical mole ration, to react with 0.124 mol of NH₃ you would need:

0.124molNH₃ × (5molCO₂/8molNH₃) = 0.0775 mol CO₂

Since there are 0.339 moles available, this is in excess.

0.124molNH₃ × (3molCH₄/8molNH₃) = 0.0465mol CO₂

Since there are 0.109 moles available, this is in excess too.

Hence, the limiting reagent is NH₃.

6. Yield

Use the theoretical ratio:

0.124molNH₃ × (4molC₂H₄N₂ / 8molNH₃) = 0.0620 mol C₂H₄N₂

Convert to grams:

Mass = number of moles × molar mass

0..0620 mol × 56.068g/mol = 3.48 g of C₂H₄N₂ ← answer

4 0

4 years ago

The particle that adds mass but no charge to the atomic nucleus is the

andrew-mc [135]

The particle that adds mass but no charge to the atomic nucleus is the neutron.

The nucleus contains both protons and neutrons.

Protons and neutrons have about the same mass.

However, protons have a positive charge, while neutrons have no charge,

6 0

4 years ago

How many moles of hydrogen sulfide are contained in a 77.7-8 sample of this gas?

valentina_108 [34]

Answer:

its either C or D my guess is C though because 35.0g of hyddrogen is =1.03 mol

Explanation:

7 0

3 years ago

When atoms from Column I (Group 1) combine with atoms from Column VII (Group 17): A nearly 100% covalent bond forms. The bond wi

gtnhenbr [62]

The answer you're looking for is B. The bond will be ionic.

7 0

3 years ago

Read 2 more answers