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Stells [14]
3 years ago
9

How many elements are there in mint chocolate chip ice cream?

Chemistry
1 answer:
Vsevolod [243]3 years ago
7 0
Well, it is a h<span>eterogeneous mixture.... but im not sure EXACTLY what you mix to get the best flavor of ice cream in the world; mint chocolate chip...</span>
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I NEED HELP WIT QUESTION THREE
mixas84 [53]

Answer: 2.00

Explanation:

2 rounded to the nearest hundredth is 2.00

your welcome :)

answers for all three:

1. 4.00

2. 16.04

3. 2.00

4 0
2 years ago
How are electrons arranged around an atom?
Schach [20]
They are arranged in shells
6 0
2 years ago
Under a certain set of conditions, the percent yield of a reaction that produces carbon dioxide is 75.0%. What mass in grams of
ExtremeBDS [4]

Answer:

Actual yield = 20.03g

Explanation:

% yield = 100.\frac{actual yield}{theoretical yield}% yield = 100. \frac{actual \ yield}{theoretical \ yield}

Actual yield = % yield.(theoretical yield) / 100

Actual yield = 75.26.7/100

Actual yield = 20.025

6 0
3 years ago
Read 2 more answers
A standard 10.00 g mass is weighed on an analytical balance 100 times. The average and standard deviation obtained gives 10.12 ±
Mekhanik [1.2K]

Answer:

There was an improvement in accuracy. There was no change in precision.

Explanation:

<em>The average mass after recalibration is closer to the mass of the standard, </em>so the recalibration improved the accuracy<em> </em>(the measurement is closer to an accepted 'true' value).

The standard deviation did not change, so the precision (or how disperse the measurements are) was not affected.

5 0
3 years ago
The free energy change for the following reaction at 25 °C, when [Cr3+] = 1.32×10-3 M and [Fe3+] = 1.14 M, is 131 kJ: Cr3+(1.32×
larisa [96]

Answer:

E°cell = - 1.3575 V

This reaction is spontaneous in the reverse direction

Explanation:

The given cell reaction:

Cr³⁺(1.32 × 10⁻³ M) + Fe²⁺(aq) → Cr²⁺(aq) + Fe³⁺(1.14 M)

The given Gibbs free energy: ΔG = 131 kJ = 131 × 10³ J     (∵ 1 kJ = 10³ J)

As we know,

ΔG = - n F E°cell

Here, n - the number of moles of electrons transferred = 1

F - Faraday constant = 96500

E°cell - cell potential = ?

\therefore E^{\circ }_{cell} = -\frac{\Delta G}{n \: F} = -\frac{131\times 10^{3}\, J}{1\, mol\times96500 \, C.mol^{-1}}

\Rightarrow E^{\circ }_{cell} = -1.3575\, V

<u>For a given chemical reaction if-</u>

1. ΔG = negative and E°cell = positive

⇒ <em>The reaction is spontaneous and proceeds spontaneously in the forward direction.</em>

2.  ΔG = positive and E°cell = negative

⇒ <em>The reaction is non-spontaneous and proceeds spontaneously in the reverse direction.</em>

<u>Since, for this chemical reaction: </u>

Cr³⁺(1.32 × 10⁻³ M) + Fe²⁺(aq) → Cr²⁺(aq) + Fe³⁺(1.14 M)

ΔG = + 131 × 10³ J ⇒ positive

and, E°cell = - 1.3575 V ⇒ negative

<u>Therefore, this reaction is spontaneous in the reverse direction.</u>

6 0
3 years ago
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