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Katarina [22]
4 years ago
13

n a certain city, electricity costs $0.18 per kW·h. What is the annual cost for electricity to power a lamp-post for 6.50 hours

per day with (a) a 100.-watt incandescent light bulb (b) an energy efficient 25-watt fluorescent bulb that produces the same amount of light? Assume 1 year = 365 days.
Chemistry
2 answers:
sveticcg [70]4 years ago
8 0

A) 100 watt = 0.1 kW  

Annual cost can be calculated as:  

Annual cost=0.1 kW ×6.50 h×365×0.13

=30.8 $

So, now the annual cost will be 30.8 $

B) 25 watt = 0.025 kW  

Annual cost can be calculated as:  

Annual cost=0.025 kW ×6.50 h×365×0.13

=7.71 $

So, now the annual cost will be 7.71 $

Bond [772]4 years ago
6 0

a)

Consumption of power in one day = 100 W \times 6.5 h = 650 Wh

Consumption of power in one year = 100 W \times 6.5 h\times 365 = 237250 Wh

Since, 1 Wh = 0.001 kWh. So,

237250 Wh = 237.25 kWh

Given that 1 kWh = $0.18

So, for 237.25 kWh:

237.25 kWh\times $ 0.18/ kWh = $42.705

Hence, the annual cost is $42.705.

b)

Consumption of power in one day = 25 W \times 6.5 h = 162.5 Wh

Consumption of power in one year = 25 W \times 6.5 h\times 365 = 59312.5 Wh

Since, 1 Wh = 0.001 kWh. So,

59312.5 Wh = 59.3125 kWh

Given that 1 kWh = $0.18

So, for 59.3125 kWh:

59.3125 kWh\times $ 0.18/ kWh = $10.676

Hence, the annual cost is $10.676.

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Soloha48 [4]

Answer:

Haven't evaporated all of the water

Explanation:

One of the main sources of error that occur in a formula of a hydrate lab is that all of the water is not evaporated. We can see at the end of the video that half of the CoCl2 is a light blue colors and the other half is a dark blue color. This indicates that all of the water still has not been evaporated off, resulting in the actual mass of the salt to be greater than the predicted value.

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3 years ago
A 7.00-mL portion of 8.00 M stock solution is to be diluted to 0.800 M. What will be the final volume after dilution? Enter your
amm1812

Explanation:

The number of moles of solute present in liter of solution is defined as molarity.

Mathematically,         Molarity = \frac{\text{no. of moles}}{\text{Volume in liter}}

Also, when number of moles are equal in a solution then the formula will be as follows.

                     M_{1} \times V_{1} = M_{2} \times V_{2}

It is given that M_{1} is 8.00 M, V_{1} is 7.00 mL, and M_{2} is 0.80 M.

Hence, calculate the value of V_{2} using above formula as follows.

                    M_{1} \times V_{1} = M_{2} \times V_{2}

                 8.00 M \times 7.00 mL = 0.80 M \times V_{2}

                      V_{2} = \frac{56 M. mL}{0.80 M}

                                  = 70 ml

Thus, we can conclude that the volume after dilution is 70 ml.

7 0
3 years ago
What is the half-life of a pharmaceutical if the initial dose is 500 mg and only 31 mg remains after 6 hours?
Sergeu [11.5K]

Answer:

\large \boxed{\text{b. 1.5 h}}

Explanation:

1. Calculate the rate constant

The integrated rate law for first order decay is

\ln \left (\dfrac{A_{0}}{A_{t}}\right ) = kt

where

A₀ and A_t are the amounts at t = 0 and t

k is the rate constant

\begin{array}{rcl}\ln \left (\dfrac{500}{31}\right) & = & k \times 6\\\\\ln 16.1 & = & 6k\\2.78& =& 6k\\k & = & \dfrac{2.78}{6}\\\\& = & 0.463 \text{ h}^{-1}\\\end{array}

2. Calculate the half-life

t_{\frac{1}{2}} = \dfrac{\ln2}{k} = \dfrac{\ln2}{\text{0.463  h}^{-1}} = \textbf{1.5 h}\\\\ \text{The half-life is $\large \boxed{\textbf{1.5 h}}$}

4 0
3 years ago
To gravimetrically analyze the silver content of a piece of jewelry made from an alloy of Ag and Cu, a student dissolves a small
Ipatiy [6.2K]

Answer:

Adding a solution containing an anion that forms an insoluble salt with only one of the metal ions.

Explanation:

The student have in solution Ag⁺ and Cu²⁺ ions but he just want to analyze the silver, that means he need to separate ions.

Centrifuging the solution to isolate the heavier ions <em>FALSE </em>Centrifugation allows the separation of a suspension but Ag⁺ and Cu²⁺ are both soluble in water.

Adding enough base solution to bring the pH up to 7.0 <em>FALSE </em>At pH = 7,0 these ions are soluble in water and its separation will not be possible.

Adding a solution containing an anion that forms an insoluble salt with only one of the metal ions <em>TRUE </em>For example, the addition of Cl⁻ will precipitate the Ag⁺ as AgCl(s) allowing its separation.

Evaporating the solution to recover the dissolved nitrates. <em>FALSE</em> . Thus, you will obtain the nitrates of these ions but will be mixed doing impossible its separation.

I hope it helps!

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