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lyudmila [28]
3 years ago
14

Four preparations involving table sugar (sucrose) are described below. Analyze the sugar preparation processes and the end produ

cts.
Sugar Water Sugar Floss Sugar Caramel Rock Sugar

Sugar is added to water, and the water is stirred until the sugar is no longer visible. Sugar is melted and blown with a fan to make thin threads of solid sugar. Pure sugar is melted and cooked until it changes color and becomes a thick, sticky liquid. A highly concentrated solution of sugar water is prepared, large sugar crystals are allowed to form slowly, and then dye is added.


Which of the following is evidence that a chemical reaction has taken place in one of the processes?
A.
the slow growth of giant sugar crystals from a highly concentrated sugar-water solution and added dye
B.
the color change that takes place after heat melts and begins to decompose the sugar
C.
the melting and re-solidification of sugar into threads, which are different from sugar’s natural cube-shaped crystals
D.
the dissolution of solid sugar in water to form a thin, colorless, odorless liquid
Chemistry
1 answer:
MAXImum [283]3 years ago
4 0

Answer:

the answer is c

Explanation:

because i got it right

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4Ag + 2H2S + O2 -> 2Ag2S + 2H20 i’m pretty sure that’s correct
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When a molecule can occupy the same active site as the substrate, a situation called __________________ can result.
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When a molecule can occupy the same active site as the substrate, a situation called enzymes can result.
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What is the standard heat of reaction for the following reaction?
8090 [49]

Answer:

The correct answer to the question is

The standard heat of reaction for the reaction is

a. 216.8 kJ released per mole

Explanation:

The heat of reaction is given by [Heat of formation of products] - [Heat of formation of reactants]

In the question we have, heat of formation of the products Zn+2 (aq) = -152.4 kJ/mole and the heat of formation of the reactants = 64.4 kJ/mole

Therefore, the heat of formation of the reaction = (-152-64.4) kJ/mole or

-216.8 kJ/mole released

5 0
3 years ago
A sample of 0.3283 g of an ionic compound containing the bromide ion (Br−) is dissolved in water and treated with an excess of A
Pavel [41]

Answer:

92.49 %

Explanation:

We first calculate the number of moles n of AgBr in 0.7127 g

n = m/M where M = molar mass of AgBr = 187.77 g/mol and m = mass of AgBr formed = 0.7127 g

n = m/M = 0.7127g/187.77 g/mol = 0.0038 mol

Since 1 mol of Bromide ion Br⁻ forms 1 mol AgBr, number of moles of Br⁻ formed = 0.0038 mol and

From n = m/M

m = nM . Where m = mass of Bromide ion precipitate and M = Molar mass of Bromine = 79.904 g/mol

m = 0.0038 mol × 79.904 g/mol = 0.3036 g

% Br in compound = m₁/m₂ × 100%

m₁ = mass of Br in compound = m = 0.3036 g (Since the same amount of Br in the compound is the same amount in the precipitate.)

m₂ = mass of compound = 0.3283 g

% Br in compound = m₁/m₂ × 100% = 0.3036/0.3283 × 100% = 0.9249 × 100% = 92.49 %

4 0
3 years ago
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