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Svetllana [295]
2 years ago
10

Determine the type of reaction: AgNO3 + Cu --> Cu(NO3)2 + Ag

Chemistry
1 answer:
guajiro [1.7K]2 years ago
7 0

Explanation:

Cu + 2 AgNO3 → Cu(NO3)2 + 2 Ag

Cu is oxidized

Ag+ is reduced

Cu is the reducing agent

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Is carbon dioxide a polar molecule? Why or Why Not?
irinina [24]

Explanation:

Carbon dioxide isn't a polar molecule because

same nature of charge appears in opposite direction which cancel each other. So, carbon dioxide is non-polar molecule.

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3 years ago
NaOH + HCl → NaCl + H2O. What mass of water forms when 2.75 × 10–4 mol NaOH reacts completely? given the equation, 2.75 × 10–4 m
Hoochie [10]
The balanced chemical reaction is written as:

<span>NaOH + HCl → NaCl + H2O

We are given the amount of sodium hydroxide to be used up in the reaction. This will be the starting point for the calculation. 

2.75 x 10^-4 mol NaOH ( 1 mol H2O / 1 mol NaOH ) ( 18.02 g H2O / 1 mol H2O ) = 4.96 x 10^-3 g H2O</span>
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3 years ago
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When K- and I- combine
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Answer:

was zum Teufel

Explanation:

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3 years ago
Why are intensive properties useful for identifying a substance?
Lesechka [4]

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d

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3 0
2 years ago
The reaction A + B → C has a ∆G'° of –20 kJ/mol at 25° C. Starting under standard conditions, one can predict that: A) at equili
Step2247 [10]

Answer:

C) at equilibrium, the concentration of C will be much greater than the concentration of A or B.  

Explanation:

A + B ⇌ C; ΔG° = -20 kJ·mol⁻¹

If ΔG is negative, the reaction is spontaneous and position of equilibrium lies to the right, so the equilibrium concentration of C is much greater than that of A or B.

A) is wrong. The molar ratio of A:B is 1:1. If their initial concentrations are 1 mol·L⁻¹, their final concentrations will be equal.

B) is wrong. The position of equilibrium lies to the right, so the concentration of C will be much greater than that of A.

D) and E) are wrong. ΔG says nothing about the rate of a reaction. It deals with the spontaneity and position of equilibrium not the speed at which equilibrium is achieved.

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2 years ago
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